1. In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture: 15 mL 2.0 M acetone + 20. mL 0.0030 M I2 + 30. mL 0.50 M HCl + 35 mL H2O (a) Calculate the number of moles of acetone in the reaction mixture. Remember M = mol/L. (b) What is the molarity of acetone in the reaction mixture (when mixed with the other chemicals)? (c) What is the molarity of HCl in the reaction mixture (when mixed with the other chemicals)?
1. In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture:
15 mL 2.0 M acetone + 20. mL 0.0030 M I2 + 30. mL 0.50 M HCl + 35 mL H2O
(a) Calculate the number of moles of acetone in the reaction mixture. Remember M = mol/L.
(b) What is the molarity of acetone in the reaction mixture (when mixed with the other chemicals)?
(c) What is the molarity of HCl in the reaction mixture (when mixed with the other chemicals)?
(d) Calculate the molarity of iodine in the reaction mixture (when mixed with the other chemicals).
(e) Figure out a way to half the molarity of acetone in the reaction mixture while keeping the total volume at 100.0 mL and keeping the concentrations of I2 and H+ ion the same as in the original mixture.
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